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What mass in grams of potassium hydroxide is contained in 500 mL of solution that has a pH of 11.5?

Your response:

[OH] = 1.0 x 0^-14 / 11.5 This isn't correct. If the pH is 11.5, then the pOH = 14 - 11.5 = 2.5 = pOH and (OH^-) = 0.00316 M. It appears to me that you have Kw mixed up with pKw.

Sorry I don't quite understand can you please do a second step?

  • chemistry -

    pH = 11.5
    pH + pOH = 14, then
    pOH = 14 - 11.5 = 2.5
    If pOH = 2.5, then (OH^-) = 0.00316 M.

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